Despite its formula, boric acid, H3BO3, is a monoprotic acid. A 25.00 mL sample of this acid required 15.66 mL of 0.1724 M NaOH to reach the equivalence point where the pH= 11.13. Determine the original concentration of boric acid and the equilibrium constant, Ka.
millimoles of NaOH = 15.66 x 0.1724 = 2.70
at equivalence point .
millimoles of acid = millimoles of base
M x 25 = 2.70
M = 0.1080
concentration of H3BO3 = 0.1080 M .
H3BO3 + NaOH ------------->
at equivalence point salt only remains. it is the salt of strong base and weak acid.
salt concentration = C = 2.70 / (15.66 + 25) = 0.06640 M
pH = 7 + 1/2 (pKa + log C)
11.13 = 7 + 1/2 (pKa + log 0.0664)
pKa = 9.438
Ka = 10^-pKa = 10^-9.438
Ka of boric acid = 3.649 x 10^-10
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